What is the Difference Between Galvanic Cell and Concentration Cell?
🆚 Go to Comparative Table 🆚The main difference between a galvanic cell and a concentration cell lies in the composition of the half-cells and their purpose:
- Galvanic Cell: A galvanic cell is a type of electrochemical cell that uses spontaneous redox reactions to generate electrical energy. It typically consists of two half-cells with different electrodes and electrolytes, and it can produce electrical energy as long as there is a driving force in the form of a spontaneous redox reaction.
- Concentration Cell: A concentration cell is a specific type of galvanic cell made of two half-cells with the same electrodes but different concentrations of the same electrolyte. The purpose of a concentration cell is to dilute the more concentrated solution and concentrate the more dilute solution, creating a voltage as the cell reaches an equilibrium by transferring electrons from the cell with the lower concentration to the cell with the higher concentration.
In summary:
Feature | Galvanic Cell | Concentration Cell |
---|---|---|
Type | Generates electrical energy through spontaneous redox reactions | Establishes equilibrium between two half-cells with the same electrodes but different concentrations |
Composition | Different electrodes and electrolytes in each half-cell | Same electrodes and electrolyte, but different concentrations in each half-cell |
Purpose | Produces electrical energy | Dilutes the more concentrated solution and concentrates the more dilute solution |
Comparative Table: Galvanic Cell vs Concentration Cell
Here is a table summarizing the differences between galvanic cells and concentration cells:
Feature | Galvanic Cell | Concentration Cell |
---|---|---|
Definition | A type of electrochemical cell that generates electrical energy through spontaneous redox reactions. | A specific type of galvanic cell where the two half-cells have the same electrodes but different concentrations. |
Electrodes | Can be made of the same or different substances. | Must be made of the same substance. |
Electrolytes | Can have the same or different electrolytes in the two half-cells. | Has identical electrodes in both half-cells. |
Concentration | Does not have the same concentration of solution on both sides. | Has the same concentration of solution on both sides, but with differing concentrations of the reacting species. |
Cell Potential | Produces a voltage that can be measured using a voltmeter. | The cell potential is dependent on concentration and can be calculated using the Nernst Equation. |
Galvanic cells involve spontaneous redox reactions to generate electrical energy, while concentration cells focus on establishing equilibrium by transferring electrons between two half-cells with the same electrodes but different concentrations. The key difference between the two is the similarity of the half-cells and their concentrations. Concentration cells are a specific type of galvanic cell with the same electrodes but different concentrations, while galvanic cells can have different electrodes and electrolytes in their half-cells.
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